Name ____________________________________________________
Chem 1 – Midterm Review Sheet
Unit 1 – Scientific Experimentation
Scientific Experimentation
1. An experiment is designed to determine where the hottest part of
a Bunsen flame is located. The height of the beaker above the
burner is varied and how long it takes for the 100mL of water to
boil is measured.
a. What is the independent variable in this experiment?
height
b. What is the dependent variable in this experiment?
c. What is a control in this experiment?
Significant Figures
1. How many significant figures are in each of the following measurements?
a. 2000 m
____________
b. 0.0025 cm
____________
c. 202 mL
____________
d. 150. kg
____________
Significant Figures in Calculations
Perform each of the following calculations and express your answer to the correct number of
significant figures.
2. 8.0g + 11.04g – 0.01g =
3. 250kg/10L =
4. 33.70cm x 0.007cm x 1200cm =
Conversion Factors
Convert each of the following measurements to the given units.
1. 5.0 L =
_________cm3
2. 0.025m =
_________um
3. 150 cm =
_________nm
4. 100in3 =
_________m3
5. A measurement has a number and a ________________.
Precision and Accuracy
The density of water was measured by three different students. Who was more precise and
accurate in his/her calculations? What was his/her accuracy? (Hint: What is the accepted value
for the density of water in g/mL?)
Trials
1
2
3
4
Jon g/mL
1.00
1.25
0.95
0.94
Jim g/mL
1.02
1.00
0.99
0.98
Joanna g/mL
1.10
0.90
0.91
1.05
Unit 2 – Properties and Classification of Matter
Chemical and Physical Changes
1. Name four evidences that indicate a chemical change has taken place.
a.
b.
c.
d.
2. Classify each of the following as a chemical change or a physical change.
a. A pile of snow gradually vaporizes.
b. Cu burns in the presence of O2 to form CuO.
c. An antacid tablet fizzes and releases carbon dioxide gas when it comes in contact with
HCl in the stomach.
d. A sugar cube dissolves in water.
3. Which of the following is a physical change?
a. burning gasoline
b. cooking an egg
c. decomposing meat
d. steam condensing on a cold bathroom mirror
e. rusting iron
4. How many of the following are compounds: table salt, carbon, copper, water, mercury?
a. 1
b. 2
c. 3
d. 4
e. 5
5. A sample of an element contains only one kind of
a. isotope b. mixture
c.atom
d.pure substance
e.none of these
6. The state of matter for an object that has neither definite shape nor definite volume is
a. solid
b. liquid
c.gaseous
d.elemental
e.mixed
Mixtures
1. Classify each of the following as mixtures or pure substances:
a. steel
b. oil and water
c. methanol
d. vinegar in water
e. a diamond
f. milk
2. Which of the mixture(s) in question 1 is/are homogeneous ? Write the letter(s) below.
3. Which of the mixture(s) in question 1 is/are a heterogeneous? Write the letter(s) below.
4. Which of the mixture(s) in question 1 is/are a colloid? Write the letter(s) below.
5. Which mixture can be separated by using the equipment
shown to the right?
a. A homogeneous solution of sugar in water
b. A heterogeneous mixture of sand and water
c. A homogeneous mixture of salt and water
Density
1. Water has a density of 1.0 g/mL. Which of the objects will float in
water?
a. Object 1: mass = 50.0 g; volume = 60.8 mL
b. Object II: mass = 65.2 g; volume = 42.1 mL
c. Object III: mass = 100.0 g; volume = 20.0 mL
a. II
b. III c. I d. II, III e. I, III
2. What volume would be occupied by a piece of aluminum (density = 2.70 g/mL) weighing 85 g?
a. 3.2 x102 mL
b. 229.5 mL
c. 3.2 mL d. 31 mL
e. none of these
Unit 3 – Che mical F ou nda tions
Element Symbols
1. The symbol for the element mercury is
a. Hg
b. Mn
c.Mg
d.Ag
e.Mr
2. Give the symbols for the following elements.
a. lead ______________
b.iron ______________ c.silver ______________
3. The law of constant composition applies to
a. metals
b. metalloids
c. homogeneous mixtures
d. heterogeneous mixtures
e. compound
Formulas
4. A substance composed of two or more elements combined chemically in a fixed proportion by
mass is a/an
a. compound
b. mixture
c. atom
d. solid
e.none of these
5. How many hydrogen atoms are indicated in the formula (NH4)2C8H 4O2?
a. 8
b. 12
c.20
d.24
e.none of these
6. The total number of oxygen atoms indicated by the formula Fe2(CO3)3 is
a. 3
b.6
c.9
d.12
e.18
Early Atomic Theory
7. The scientist whose alpha-particle scattering experiment led him to conclude that the nucleus
of an atom contains a dense center of positive charge is
a. J. J. Thomson
b. Lord Kelvin
c. Ernest Rutherford
d. William Thomson
e. James Chadwick
Atomic Structure
8 . How many protons, electrons, and neutrons respectively does
a.
b.
c.
d.
e.
53,
53,
53,
74,
53,
127, 74
74, 53
53, 127
53, 127
53, 74
9. The number of neutrons in one atom of
a. 82
b. 206
c.124
206
Hg
82
is
d.288
127
I have?
10. Which of the following compounds are ionic?
a. MgO
b. SO3
c. HCl
d. CO2
Periodic Table
11. Which of the following elements is an alkali metal?
a. Ca
b. Cu
c. Fe
d. Na
e. Sc
12. Halogens exist naturally as these types of molecules.
e. Monatomic
f. Diatomic
g. Elements
h. Ionic
13. Which of the following elements is most chemically similar to Ca?
a. Na
b. N
c. O
d. Mg
e. C
14. Rows of the periodic table are called? ____________________________________
15. Columns of the periodic table are called? _________________________________
Unit 4 – Modern Atomic Theory
EM Radiation
1. The form of EMR that has more energy per photon than X-rays is
i.
j.
k.
l.
m.
microwaves
radio waves
gamma rays
infrared rays
none of these
2. The energy levels of the hydrogen atom (and all atoms) are ______________, meaning that only certain
discrete energy levels are allowed.
a. varied
b. quantized
c. ramp-like
d. continuous
e. two of these
3. The form of EMR that has less energy per photon than microwaves is
a.
microwaves
b.
radio waves
c.
gamma rays
d.
infrared rays
e.
none of these
4. ______________ is a form of oxygen that protects us from high-energy radiation emitted by the sun.
a. Ozone
b. Carbon dioxide
c. Ultraviolet light
d. Methane
e. None of these
Atomic Orbitals
1. The probability map for an electron is called a/an
a.
orbit
b.photon
c. orbital
d. electron configuration
e. none of these
2. As the principal energy level increases in an atom, the average distance of an electron from the nucleus _.
a. increases
b. decreases c. stays the same
d. varies
e. none of these
3. The shape of an s orbital is
a. spherical
b.dumbbell shaped
c. donut shaped
4 A given set of p orbitals consists of ______________ orbital(s).
a. 1
b. 2
c. 3
d. 4
e.5
5. The maximum number of electrons allowed in ea ch of the p orbitals is
a. 2
b. 4
c. 8
d. 18 e. none of these
6. A given set of d orbitals consists of ______________ orbital(s).
a. 1
b. 3
c. 5
d. 6
e. none of these
7. The maximum number of electrons allowed in ea ch of the d orbitals is
a. 2
b. 4
c. 8
d. 18 e. none of these
Electron Configurations
1. Sodium has how many electrons in its outermost principal energy level?
a. 1
b. 2
c. 6
d. 8
e. 11
2. The number of unpaired electrons in an oxygen atom is
a. 1
b. 2
c. 3
d. 4
e. 5
3. The
a.
b.
c.
d.
e.
electron configuration for the phosphorus atom is
1s 22s 22p 63s 23p 3
1s 22s 22p 63s 23p 64s 1
1s 22s 22p 63s 5
1s 22s 22p 63p 5
none of these
4. The
a.
b.
c.
d.
e.
electron configuration for the carbon atom is
1s 22s 22p 2
[He] 2s 4
[Ne] 2s 22p 2
1s 22p 4
none of these
d. conical shaped
5. When moving down a group (family) in the periodic table, the number of valence electrons
a. remains constant
b. increases by 2 then 8 then 18 then 32
c. doubles with each move
d. decreases regularly
e. changes in an unpredictable manner
6. The element with the electron configuration [Kr] 5s 24d 105p 3 is
a. As
b. Sb
c. Nb
d. Pr
e. none of these
Atomic Trends
1. Which of the following atoms has the largest atomic radius?
a. Na
b. Mg
c. Si
d. P
e. C
2.
Which of the following atoms has the highest ionization energy?
a. N
b. Mg
c. Si
d. P
e. Cl
Bonding
1. When electrons are shared unequally, chemists characterize these types of bonds as ______________.
a) polar covalent b) ionic
c) pure covalent d) unbalanced
e) none of these
2. Chemical bonds formed by the attraction of oppositely charged ions are called
a) covalent bonds b) magnetic bonds c) coordinate bonds d) ionic bonds e) none of these
3. Which of the following compounds contains one or more covalent bonds?
a) NaCl
b) CaO
c) CO2
d) Cs2 O
e) BaBr
4. Which element or ion listed below has the electron configuration 1s22s22p 6 3s23p 6?
a) Cl
b) Brc) Se
d) Ca2+
e) two of these
5. A phosphorus atom needs to gain ______________ electrons to achieve a noble gas configuration.
a) 2 b) 3 c) 4 d) 5 e) 6
6. How many lone pairs of electrons are in the Lewis structure for ammonia, NH3?
a) 0
b) 1
c) 2
d) 3
e) 4
7. What is the geometry of NH3?
a) linear b. bent
c. trigonal pyramidal
d. trigonal planar
e. tetrahedral
8. Which of the following has a double bond?
a) H2 O
b) C2H2
c) C2H4
d) CN-
e) none of these
9. What is the correct order of the following bonds in terms of decreasing polarity?
a) N--Cl, P--Cl, As--Cl
b) P--Cl, N--Cl, As--Cl
c) As--Cl, N--Cl, P--Cl
d) P--Cl, As--Cl, N--Cl
e) As--Cl, P--Cl, N—C
Chemical Nomenclature
1. Which of the following is a binary compound?
a) O2
b) HCN
c) H2SO4
d) H2S
e) NaOH
2. The correct name for LiCl is
a) lithium monochloride
b) lithium(I) chloride
c) monolithium chloride
d) lithium chloride
e) monolithium monochloride
3. The correct name for P2 O 5 is
a) phosphorus(II) oxide
b) phosphorus(V) oxide
c) diphosphorus oxide
d) diphosphorus pentoxide
e) phosphorus pentoxide
4. The binary compound PbCl2 is called
a) Lead chloride
b) Lead (II) chloride
c) Lead (II) chlorate
d) Lead dichloride
e) none of these